Information

Extension

1163

Email address

mcquades at ollchs dot org

Photo 1

Teachers & Homework

Ms. Stephanie McQuade

Department: Science

Ms. McQuade has been teaching for over 5 years after earning a BS in Chemistry from Binghamton University as well as an MAT in Chemistry Education from Binghamton University.  She teaches Regents, Honors and AP Chemistry.  She is also the JV Volleyball coach and the senior class advisor.

AP Chem-Ms. McQuade

Extra Help for the week of 2/18- 2/21
2/18-2/21/14

Extra Help this week will be
Tuesday AP Chem- 3pm Room 106
Wednesday- Regents and Honors Chem 3pm Room 106
Thursday- Honors lab make up/ Regents and Honors extra help 3pm - Chem Lab

Extra Help for the week of 11/18-22
11/18/13-11/22/13

Extra Help this week will be:
Monday 3:00-3:30pm and Thursday 3:00-3:30pm or by appointment

Atomic Theory Notes

Atomic Theory notes in pdf if you need them
Atomic_Theory_notes.pdf

Online registration
9/13/13

Sorry for the confusion.  Lets try using the url
1. go to www.pearsonschool.com/access
2. enter the access code SSNAST-WHIRR-RABIC-CLIMB-HELOT-SOUSE
3. Select our textbook from the drop down menu (Brown and LeMay 12th edition)
4. Follow the instructions for creating an account.  Course code: OLLAPChem

Please email me when you have registered or if there are still problems.

Mastering Chemistry Registration
9/12/13

You need to register for Mastering Chemistry.  This is the online program we will be using for homework. 
go to http://www.masteringchemistry.com/site/index.html and click the Student box under register.  Your access code is:
SSNAST-WHIRR-RABIC-CLIMB-HELOT-SOUSE
and your course code is OLLAPChem
if you need help watch this video
http://www.youtube.com/watch?v=BCWgNu-kxi0&list=PLRpRY65o3rxaYHYB9UC-_rOeB1yaU93wz&index=2


the how to introduction HW is Due Monday 9/16 by noon.

Student Information Sheet
9/12/11

Complete youe Student Information sheet

Chem H-Ms. McQuade

OB Kinetics
Due 4/7

In your orange book read p 136-141 and answer questions 1-17

Limiting Reactant WS
3/25/14

Complete the Limiting Reactant WS.  Follow the steps on the top of the sheet to determine the grams of product.

Solutions Test
Tuesday 3/24

TEST HAS BEEN MOVED TO WEDNESDAY 3/26
SOLUTIONS

At the conclusion of this unit, you should be able to:

1. Define solution, solute, and solvent
2. Identify the solute and solvent of a solution
3. Describe the factors that determine the rate of dissolving
4. Define solubility
5. Describe the difference in solubility curves for a solids and a gas
6. Describe the process of dissolving and precipitation from a molecular perspective
7. Define solution equilibrium
8. Define and identify saturated, unsaturated and supersaturated solutions
9. Describe the solubility rule in terms of polarity
10. Describe the effects of pressure and temperature on the solubility of a gas
11. Use Table F and Table G on the Reference Table
12. Differentiate between concentrated and dilute solutions
13. Describe the various ways to measure the concentration of a solution
14. Calculate the molarity of a solution
15. Calculate the concentration of a solution using parts per million (ppm)
16. Describe the impact of solutes on vapor pressure, freezing point and boiling point of a liquid


Solutions_Review_Packet.pdf

Orange Book p111
3/10/14

In your Orange book read the bond type section on p 110-111
Copy the chart into your notebook
Answer questions 38-44

Solutions Handout
3/7/14

Read and answer questions

Chemical Reactions and Moles Test
3/6/14

UNIT SIX OBJECTIVES

MOLES AND CHEMICAL REACTIONS

At the conclusion of this unit, you should be able to:

1. Explain what information can be derived from a chemical formula
2. Differentiate between binary and ternary compounds
3. Name compounds using the IUPAC system of nomenclature
4. Write the formula of compounds given their IUPAC names
5. Convert word equations into chemical equations using symbols
6. Identify the number of atoms in a compound
7. Given the chemical equation of a chemical reaction, classify it into one of the four basic types: single replacement, double replacement, synthesis, or decomposition
8. Differentiate between reactants and products of a chemical equation
9. Define Law of Conservation of Matter
10. Balance simple chemical equations
11. Describe the role of coefficients in a chemical equation
12. Determine the mole ratio of the reactant and/or product using a balanced equation
13. Calculate the moles of products that should be formed given the moles of reactant consumed
14. Calculate the formula mass of a compound
15. Determine the percent composition, by mass, of an element in a compound
16. Define mole and describe it importance in chemistry
17. Differentiate between formula mass (amu) and gram formula mass (g)
18. Convert the mass of a compound into the mole of the compound
19. Convert the moles of a compound into the mass of the compound
20. Determine empirical formula from molecular formula.
21. Determine molecular formula when given empirical formula and formula mass. 
22. Determine the percent composition of water in a hydrated salt

The review packet is posted below.  Answers appear on the last page. 
Reactions_and_Moles_Review_Packet.pdf

Percent composition WS
2/20/14

Complete the front and back of the percent composition WS.

Extra Help for the week of 2/18- 2/21
2/18-2/21/14

Extra Help this week will be
Tuesday AP Chem- 3pm Room 106
Wednesday- Regents and Honors Chem 3pm Room 106
Thursday- Honors lab make up/ Regents and Honors extra help 3pm - Chem Lab

Formula Mass WS
2/18/14

Determine the formula mass of each compound. 
a big dot before H2O indicates a salt bonded to waters.  Add the mass of salt to water (DO NOT MULTIPLY the mass of the salt by the mass of the water).

Bonding Test
1/17/14

BONDING

At the conclusion of this unit, you should be able to:

1. Define a chemical bond
2. Differentiate between ionic bonding and covalent bonding
3. Define electronegativity and use the electronegativity difference to determine the character of the bond between two elements
4. Differentiate between polar covalent bond and nonpolar covalent bond
5. Define molecule, molecular compound, and diatomic molecule
6. Describe the change in potential energy as a chemical bond is formed
7. State the octet rule and explain the rule based on electron configuration and potential energy
8. Draw the Lewis-electron dot diagram of an element and how it relates to valence electrons
9. Draw the Lewis structures of basic molecular compounds
10. Describe the shape and polarity of common molecules
11. Describe the factors that determine the overall polarity of a molecule
12. Differentiate among single bond, double bond and triple bond
13. Define dipole, and describe dipole-dipole forces
14. Define hydrogen bonding
15. Describe how boiling points and melting points are dictated by bond types
16. Define ionic compound and contrast its properties from molecular compounds
17. Draw the Lewis dot diagram of a ionic compounds
18. Define metallic bonding and identify properties of metals
19. Differentiate between intermolecular forces and intramolecular forces
20. Explain what information can be derived from a chemical formula
21. Name compounds using the IUPAC system of nomenclature
22. Write the formula of compounds given their IUPAC names

Review Packet will be checked on Thursday 1/16/14. Answers are on the last page of the pdf below
CBonding_Review_Packet.pdfHEMICAL

 

 

Bonding Vocab
12/10/13

On p 206 in the text book is the list of terms to define from chapter 7

Periodic Table Test
12/5/13

Periodic_Table_Review_Packet.pdf

THE PERIODIC TABLE

At the conclusion of this unit, you should be able to:

1. Describe the evolution of the periodic table and contribution of Mendeleev
2. Identify metals and nonmetals on the periodic table.
3. List characteristics of metals and nonmetals
4. Define luster, melting point, boiling point, ductility, malleability, electrical conductivity, and thermal conductivity
5. Differentiate between groups and periods of the periodic table
6. List seven diatomic elements
7. Describe the arrangement of the periodic table based on electron configuration
8. Describe the physical and chemical properties of selected groups of the periodic table (Groups 1, 2, 17 and 18)
9. Describe the characteristics of elements in group on the periodic table
10. Define atomic radii, ionization energy, valence electrons, metallic character, and electronegativity
11. Describe the trends or patterns of the above terms across the periodic table
12. Compare the size of an atom to its ion
13. Identify the state of matter of an element at Standard Temperature using Table S

Periodic Project
Due 12/3

Using the attached rubric complete an element tile for your assigned element
Periodic_Project.doc

6.1
11/26/13

In your textbook read p 155-160 and complete questions 1-7 on p 160

“Trendy Lab” discussion of Theory
11/20/13

A few sentences tying the concepts in class to the lab.  This should be about 4-5 sentences and key terms should be defined and explained.  Including but not limited to Periodic Table, Group, Period, Electronegativity , first ionization energy and atomic radius

Orange book Periodic Table
11/20/13

In the Orange Review Book Read p 85-90 and answer questions 30-42

Extra Help for the week of 11/18-22
11/18/13-11/22/13

Extra Help this week will be:
Monday 3:00-3:30pm and Thursday 3:00-3:30pm or by appointment

Periodic Table Vocab
11/18/13

Define the following terms
Periodic Table
Period
Group
Atomic Radius
First Ionization Energy
Electronegativity
Metal
Nonmetal
Mettaloid (semi-metal)
malleable
brittle
conductive
luster

Atomic Theory Test
11/14/13

Atomic_Theory_Test_Review_Packet.pdf


UNIT FOUR OBJECTIVE SHEET

ATOMIC STRUCTURE

At the conclusion of this unit, you should be able to:

1. Define atom and identify the two regions of an atom
2. Describe the three subatomic particles in terms of mass, charge, and location
3. Given the mass and charge of an element, determine the number of protons, electrons and neutrons
4. Distinguish between isotopes of an element and recognize symbol notation.
5. Calculate the average atomic mass given the isotopes’ relative abundance
6. Describe the contributions of Dalton, Thomson, Rutherford, and Bohr
7. Describe Rutherford’s famous gold foil experiment
8. Describe the evolution of the atomic model
9. Describe the wave-mechanical model of the atom
10. Differentiate between the ground state and excited state of an atom
11. Define spectral lines and explain how they are formed
12. Define electron configuration
13. Define valence electron and define the number of valence electrons of an element.
14. Define atomic number and atomic mass in terms of subatomic particles.
15. Recognize electron configurations in the ground state and in the excited state.
16. Determine the number of electrons in an ion.
17. *Define energy levels, the Aufbau principle, Heisenberg’s uncertainty principle and Hund’s rule as they apply to energy level diagrams
18. *Assign electron configurations to elements using the s,p,d,f sublevel notation.  This includes knowing the order of filling and the maximum number of electrons at each sublevel.   

*Denotes Honors material

Electron Configuration WS
11/6/13

Complete the electron configuration WS. Note excited state and ion configurations

Atomic Notations WS (Chart)
11/1/13

Complete the atomic notation chart ws

Chap 4 Vocab
10/23 (Honors) 10/24(Regents)

in your textbook define the vocabulary from chapter 4

Atomic Theory handout
10/22 Honors 10/23 Regents

Read and answer the questions to the Atomic Theory handout

Gas Laws Questions
10/11/13

Answers to the supplemental gas laws questions.
1. 0.667atm
2. 3.69L
3. 2.42atm= 245.34kPa
4. 2.13 mol
5. Ne and CH4
6. 0.125L
7. 83.3mL
8. The moles of He equal the moles of nitrogen
9. 2.5L

Gas Laws Review Answers
10/11/13

Answers the the Gas Laws Review HW
1. Inverse graph
2.a. 2.8atm
b. as the volume decreases the particles have less room the move and collide more often.
3. Particles slow down
4. 99.1L
5. -21C
6. 0.45atm
7. it needs to be cool out.  (low pressure outside of the balloon, high pressure inside of the balloon. 
8. 106.27kPa
9. 145C
10. 47.16 L
11. as the temperature increases the volume increases. 
12. 298K and 283K
13. 2.37L
14. The particles slowed down and got closer together. 

Gas Laws Quiz
10/17/13

HONORS CHEMISTRY
UNIT TWO OBJECTIVES

GAS LAWS

At the conclusion of this unit, you should be able to:

1. Identify the different scales for measure temperature
2. Convert between Celsius and Kelvin
3. Describe the relationship, mathematically, verbally and graphically, between the volume of a gas and its absolute temperature
4. Describe the relationship, mathematically, verbally and graphically, between the volume of a gas and pressure
5. Solve gas law problems using the combined gas law
6. Differentiate between ideal gases and real gases
7. * Solve gas law problems using the ideal gas equation

*Denotes honors material not on the Regents

Gas Laws Review
10/11/13

Complete the gas laws review Questions using the combined gas law

Gas Laws Handout
10/4/13

Read and complete the gas laws handout.  You will need to use your textbook.  Answers begin on p 418

Chapter 2
9/30/13

Read section 2.1, 2.2, 2.3, 2.4 in the text book and answer questions
2.1 # 1-4
2.2 # 11-12
2.3 # 20-22
2.4 # 28-30

Matter and Energy Test
10/2/13

STUDY FOR THE MATTER AND ENERGY TEST

At the conclusion of this unit, you should be able to:

1. Define chemistry
2. Define matter
3. Differentiate between a physical property and a chemical property
4. Define and differentiate between mixture and pure substance
5. Differentiate between a homogeneous mixture and a heterogeneous mixture
6. Define element and compound
7. Classify an example as an element, compound, or mixture
8. Describe the process of chromatography, evaporation, filtration, and distillation
9. Define luster, melting point, boiling point, malleability,
10. Calculate the density of an object given its mass and volume
11. Determine the volume of by using the water displacement method
12. Calculate percent error
13. Define energy and distinguish between potential energy and kinetic energy
14. Differentiate between endothermic and exothermic process
15. Define the law of conservation of energy
16. Explain the properties of solids using the kinetic molecular theory of matter
17. Explain the properties of liquids using the kinetic molecular theory of matter
18. Explain the properties of gases using the kinetic molecular theory of matter
19. Explain the process of melting, freezing, vaporization, and condensation in terms of particle behavior
20. Define specific heat capacity
21. Describe the process of calorimetry and calculate the heat change given the mass and temperature change of a sample of water.
22. Draw the heating curve of a substance as it undergoes a phase change
23. Identify the melting point and boiling point of a substance given the heating or cooling curve
24. Calculate the heat energy needed to melt a sample of ice or vaporize a sample of water

 

Heat equations Worksheet
9/25/13

use the heat equations to answer the questions.  Constants are on able B and listed on the HW.

The golden crown
9/24/13

Read and answer the questions.  The_Golden_Crown.doc

Matter and Energy Quiz
9/23/13

Quiz on Matter and Energy including:
States of matter
Energy and Energy changes
Phase changes
heating curve

Heating Curve worksheet
9/20/13

Complete the heating curve WS

Chap 13 Section 2
9/18/13

Read section 13.2 (p 390-395) and answer questions 8-11

Chap 13 section 1
9/17/13

Read section 13.1 in the text (p385-389) and answer questions 1-6 on pages 387-9

Matter and Energy Vocab
9/16/13

Complete the vocab HW using your text or another valid source

Lab Safety
9/13/13

Lab Safety contract must be signed by student and a parent.

Lab equipment notes must be completed.

Student Information Sheet
9/12/11

Complete youe Student Information sheet

Chemistry R - Stephanie McQuade

OB Kinetics
Due 4/7

In your orange book read p 136-141 and answer questions 1-17

Concentration of solutions
3/25/14

handout_(molarity).doc

Determine the concentration using formulas from table T. Questions with and * denote a 2 step question.

Solutions Test
Tuesday 3/24

TEST HAS BEEN MOVED TO WEDNESDAY 3/26
SOLUTIONS

At the conclusion of this unit, you should be able to:

1. Define solution, solute, and solvent
2. Identify the solute and solvent of a solution
3. Describe the factors that determine the rate of dissolving
4. Define solubility
5. Describe the difference in solubility curves for a solids and a gas
6. Describe the process of dissolving and precipitation from a molecular perspective
7. Define solution equilibrium
8. Define and identify saturated, unsaturated and supersaturated solutions
9. Describe the solubility rule in terms of polarity
10. Describe the effects of pressure and temperature on the solubility of a gas
11. Use Table F and Table G on the Reference Table
12. Differentiate between concentrated and dilute solutions
13. Describe the various ways to measure the concentration of a solution
14. Calculate the molarity of a solution
15. Calculate the concentration of a solution using parts per million (ppm)
16. Describe the impact of solutes on vapor pressure, freezing point and boiling point of a liquid


Solutions_Review_Packet.pdf

Orange Book p111
3/10/14

In your Orange book read the bond type section on p 110-111
Copy the chart into your notebook
Answer questions 38-44

Solutions Handout
3/7/14

Read and answer questions

Chemical Reactions and Moles Test
3/6/14

UNIT SIX OBJECTIVES

MOLES AND CHEMICAL REACTIONS

At the conclusion of this unit, you should be able to:

1. Explain what information can be derived from a chemical formula
2. Differentiate between binary and ternary compounds
3. Name compounds using the IUPAC system of nomenclature
4. Write the formula of compounds given their IUPAC names
5. Convert word equations into chemical equations using symbols
6. Identify the number of atoms in a compound
7. Given the chemical equation of a chemical reaction, classify it into one of the four basic types: single replacement, double replacement, synthesis, or decomposition
8. Differentiate between reactants and products of a chemical equation
9. Define Law of Conservation of Matter
10. Balance simple chemical equations
11. Describe the role of coefficients in a chemical equation
12. Determine the mole ratio of the reactant and/or product using a balanced equation
13. Calculate the moles of products that should be formed given the moles of reactant consumed
14. Calculate the formula mass of a compound
15. Determine the percent composition, by mass, of an element in a compound
16. Define mole and describe it importance in chemistry
17. Differentiate between formula mass (amu) and gram formula mass (g)
18. Convert the mass of a compound into the mole of the compound
19. Convert the moles of a compound into the mass of the compound
20. Determine empirical formula from molecular formula.
21. Determine molecular formula when given empirical formula and formula mass. 
22. Determine the percent composition of water in a hydrated salt

The review packet is posted below.  Answers appear on the last page. 
Reactions_and_Moles_Review_Packet.pdf

Percent composition WS
2/20/14

Complete the front and back of the percent composition WS.

Extra Help for the week of 2/18- 2/21
2/18-2/21/14

Extra Help this week will be
Tuesday AP Chem- 3pm Room 106
Wednesday- Regents and Honors Chem 3pm Room 106
Thursday- Honors lab make up/ Regents and Honors extra help 3pm - Chem Lab

Formula Mass WS
2/18/14

Determine the formula mass of each compound. 
a big dot before H2O indicates a salt bonded to waters.  Add the mass of salt to water (DO NOT MULTIPLY the mass of the salt by the mass of the water).

Chapter 10 work
2/13/14

In your textbook read sections 10.1 and 10.2 and answer the Key concept questions. 
Define the Chapter 10 Vocabulary.

Bonding Test
1/17/14

BONDING

At the conclusion of this unit, you should be able to:

1. Define a chemical bond
2. Differentiate between ionic bonding and covalent bonding
3. Define electronegativity and use the electronegativity difference to determine the character of the bond between two elements
4. Differentiate between polar covalent bond and nonpolar covalent bond
5. Define molecule, molecular compound, and diatomic molecule
6. Describe the change in potential energy as a chemical bond is formed
7. State the octet rule and explain the rule based on electron configuration and potential energy
8. Draw the Lewis-electron dot diagram of an element and how it relates to valence electrons
9. Draw the Lewis structures of basic molecular compounds
10. Describe the shape and polarity of common molecules
11. Describe the factors that determine the overall polarity of a molecule
12. Differentiate among single bond, double bond and triple bond
13. Define dipole, and describe dipole-dipole forces
14. Define hydrogen bonding
15. Describe how boiling points and melting points are dictated by bond types
16. Define ionic compound and contrast its properties from molecular compounds
17. Draw the Lewis dot diagram of a ionic compounds
18. Define metallic bonding and identify properties of metals
19. Differentiate between intermolecular forces and intramolecular forces
20. Explain what information can be derived from a chemical formula
21. Name compounds using the IUPAC system of nomenclature
22. Write the formula of compounds given their IUPAC names

Review Packet will be checked on Thursday 1/16/14. Answers are on the last page of the pdf below
CBonding_Review_Packet.pdfHEMICAL

 

 

Bonding Vocab
12/10/13

On p 206 in the text book is the list of terms to define from chapter 7

Periodic Table Test
12/5/13

Periodic_Table_Review_Packet.pdf

THE PERIODIC TABLE

At the conclusion of this unit, you should be able to:

1. Describe the evolution of the periodic table and contribution of Mendeleev
2. Identify metals and nonmetals on the periodic table.
3. List characteristics of metals and nonmetals
4. Define luster, melting point, boiling point, ductility, malleability, electrical conductivity, and thermal conductivity
5. Differentiate between groups and periods of the periodic table
6. List seven diatomic elements
7. Describe the arrangement of the periodic table based on electron configuration
8. Describe the physical and chemical properties of selected groups of the periodic table (Groups 1, 2, 17 and 18)
9. Describe the characteristics of elements in group on the periodic table
10. Define atomic radii, ionization energy, valence electrons, metallic character, and electronegativity
11. Describe the trends or patterns of the above terms across the periodic table
12. Compare the size of an atom to its ion
13. Identify the state of matter of an element at Standard Temperature using Table S

Periodic Project
Due 12/3

Using the attached rubric complete an element tile for your assigned element
Periodic_Project.doc

6.1
11/26/13

In your textbook read p 155-160 and complete questions 1-7 on p 160

Orange book Periodic Table
11/20/13

In the Orange Review Book Read p 85-90 and answer questions 30-42

Extra Help for the week of 11/18-22
11/18/13-11/22/13

Extra Help this week will be:
Monday 3:00-3:30pm and Thursday 3:00-3:30pm or by appointment

Periodic Table Vocab
11/18/13

Define the following terms
Periodic Table
Period
Group
Atomic Radius
First Ionization Energy
Electronegativity
Metal
Nonmetal
Mettaloid (semi-metal)
malleable
brittle
conductive
luster

Atomic Theory Test
11/14/13

Atomic_Theory_Test_Review_Packet.pdf


UNIT FOUR OBJECTIVE SHEET

ATOMIC STRUCTURE

At the conclusion of this unit, you should be able to:

1. Define atom and identify the two regions of an atom
2. Describe the three subatomic particles in terms of mass, charge, and location
3. Given the mass and charge of an element, determine the number of protons, electrons and neutrons
4. Distinguish between isotopes of an element and recognize symbol notation.
5. Calculate the average atomic mass given the isotopes’ relative abundance
6. Describe the contributions of Dalton, Thomson, Rutherford, and Bohr
7. Describe Rutherford’s famous gold foil experiment
8. Describe the evolution of the atomic model
9. Describe the wave-mechanical model of the atom
10. Differentiate between the ground state and excited state of an atom
11. Define spectral lines and explain how they are formed
12. Define electron configuration
13. Define valence electron and define the number of valence electrons of an element.
14. Define atomic number and atomic mass in terms of subatomic particles.
15. Recognize electron configurations in the ground state and in the excited state.
16. Determine the number of electrons in an ion.
17. *Define energy levels, the Aufbau principle, Heisenberg’s uncertainty principle and Hund’s rule as they apply to energy level diagrams
18. *Assign electron configurations to elements using the s,p,d,f sublevel notation.  This includes knowing the order of filling and the maximum number of electrons at each sublevel.   

*Denotes Honors material

Orange Book
11/6/13

Orange book page 11. Answer questions 13-28

Atomic Theory Quiz
11/4/13

30 point Quiz on Atomic Structure
To be sucessfull you should be able to:
1. Define atom and identify the two regions of an atom
2. Describe the three subatomic particles in terms of mass, charge, and location
3. Given the mass and charge of an element, determine the number of protons, electrons and neutrons
4. Distinguish between isotopes of an element
5. Describe the contributions of Dalton, Thomson, Rutherford, and Bohr
6. Describe Rutherford’s famous gold foil experiment
7. Describe the evolution of the atomic model
8. Differentiate between the ground state and excited state of an atom
11. Define spectral lines and explain how they are formed
12. Define electron configuration
14. Define atomic number and atomic mass in terms of subatomic particles.

 

Chap 4 Vocab
10/23 (Honors) 10/24(Regents)

in your textbook define the vocabulary from chapter 4

Atomic Theory handout
10/22 Honors 10/23 Regents

Read and answer the questions to the Atomic Theory handout

Sig Fig Questions
12/22/13

In the Orange review book.
Appendix p A-20 #14-34

Gas Laws Review Answers
10/11/13

Answers the the Gas Laws Review HW
1. Inverse graph
2.a. 2.8atm
b. as the volume decreases the particles have less room the move and collide more often.
3. Particles slow down
4. 99.1L
5. -21C
6. 0.45atm
7. it needs to be cool out.  (low pressure outside of the balloon, high pressure inside of the balloon. 
8. 106.27kPa
9. 145C
10. 47.16 L
11. as the temperature increases the volume increases. 
12. 298K and 283K
13. 2.37L
14. The particles slowed down and got closer together. 

Gas Laws Quiz
10/17/13

REGENTS CHEMISTRY
UNIT TWO OBJECTIVES

GAS LAWS

At the conclusion of this unit, you should be able to:

1. Identify the different scales for measure temperature
2. Convert between Celsius and Kelvin
3. Describe the relationship, mathematically, verbally and graphically, between the volume of a gas and its absolute temperature
4. Describe the relationship, mathematically, verbally and graphically, between the volume of a gas and pressure
5. Solve gas law problems using the combined gas law
6. Differentiate between ideal gases and real gases

Gas Laws Review
10/17/13

Complete the gas laws review sheet using the combined gas law

Gas Laws Worksheet
10/11/13

Complete the gas laws worksheet using the combined gas law.

Gas Laws Handout
10/4/13

Read and complete the gas laws handout.  You will need to use your textbook.  Answers begin on p 418

Matter and Energy Test
10/2/13

STUDY FOR THE MATTER AND ENERGY TEST

At the conclusion of this unit, you should be able to:

1. Define chemistry
2. Define matter
3. Differentiate between a physical property and a chemical property
4. Define and differentiate between mixture and pure substance
5. Differentiate between a homogeneous mixture and a heterogeneous mixture
6. Define element and compound
7. Classify an example as an element, compound, or mixture
8. Describe the process of chromatography, evaporation, filtration, and distillation
9. Define luster, melting point, boiling point, malleability,
10. Calculate the density of an object given its mass and volume
11. Determine the volume of by using the water displacement method
12. Calculate percent error
13. Define energy and distinguish between potential energy and kinetic energy
14. Differentiate between endothermic and exothermic process
15. Define the law of conservation of energy
16. Explain the properties of solids using the kinetic molecular theory of matter
17. Explain the properties of liquids using the kinetic molecular theory of matter
18. Explain the properties of gases using the kinetic molecular theory of matter
19. Explain the process of melting, freezing, vaporization, and condensation in terms of particle behavior
20. Define specific heat capacity
21. Describe the process of calorimetry and calculate the heat change given the mass and temperature change of a sample of water.
22. Draw the heating curve of a substance as it undergoes a phase change
23. Identify the melting point and boiling point of a substance given the heating or cooling curve
24. Calculate the heat energy needed to melt a sample of ice or vaporize a sample of water

 

Heat Problems WS
9/26/13

Use the heat equations to solve each heat problem. 
q=mcDeltaT for temperature change
q=mhf for freezing/melting
q=mHv for vaporization and condensation

use GPS to find the answer
Givens
Plug in
Solve

The Golden crown
9/25/13

Read and answer the questionsThe_Golden_Crown.doc

Chapter 17 section1
9/23/13

In the text book read section 17.1 (p 505-510) and complete questions 5-8 on p 210

Matter and Energy Quiz
9/24/13

Quiz on Matter and Energy including:
States of matter
Energy and Energy changes
Phase changes
heating curve

Heating Curve worksheet
9/20/13

Complete the heating curve WS

Chapter 13 sections 1 and 2
9/18/13

In your text book read sections 13.1 and 13.2 and answer question 3,4,5,8,and 9 on pages 389 and 395

Lab Contract and Equiptment
9/16/13

Lab Safety contract must be signed by student and a parent.
Lab equipment notes must be completed.

Student Information Sheet
9/12/11

Complete youe Student Information sheet

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